Solutions & Concentrations

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View and manipulate the simulation to answer the following questions. http://phet.colorado.edu/sims/html/concentration/latest/concentration_en.html

Name: (last, first) *

e-mail address: *

Which action(s) will increase the concentration of the solution? (1) Add more Co(NO3)2 (2) Evaporate water (3) Drain solution *

(1) only

(1) and (2)

(2) and (3)

(1) and (3)

(1), (2), and (3)

Coblalt (II) nitrate: Co(NO3)2

Which action(s) will change the number of moles of solute in the container? (1) Add more Co(NO3)2 (2) Evaporate water (3) Drain solution *

(1) only

(1) and (2)

(2) and (3)

(1) and (3)

(1), (2), and (3)

What will happen to the concentration and the number of moles when water is added? Molarity (M) = Moles solute / Liter solution *

concentration: increases; # of moles: decreases

concentration: increases; # of moles: remains constant

concentration: no change; # of moles: increases

concentration: decreases; # of moles: decreases

concentration: increases; # of moles: increases

concentration: decreases; # of moles: remains constant

How many moles of solute are in the beaker? Molarity (M) = Moles solute / Liter solution *

0.05 moles

0.25 moles

0.50 moles

1.00 moles

2.50 moles

You are given 200 mL of a 0.400 M solution of KMnO4. If you add water until total volume is 800 mL, what will be the final concentration of the solution? Molarity (M1) x Volume (V1) = Molarity (M2) x Volume (V2) *

0.080M

0.10 M

0.20 M

0.40 M

1.6 M

Potassium permanganate: KMnO4

You start with 0.1 L of a 5.00 M solution of NiCl2, and you plan to dilute it (by adding water) to make a solution with a concentration of 0.625 M. How far should you fill the beaker? Molarity (M1) x Volume (V1) = Molarity (M2) x Volume (V2) *

200 mL

400 mL

600 mL

800 mL

1 Liter

Nickel (II) chloride: NiCl2

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